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![The Preference of Oxygen Groups
Table 1. Data Of Some Oxygen Group Characteristic
elements Electron Melting Boiling point
configuration point (oC) (oC)
8O [2He] 2s2 2p4 -219 -183
16S [10Ne] 3s2 3p4 119 445
34Se [18Ar] 3d10 4s2 4p4 221 685
52Te [36Kr] 4d10 5s2 5p4 452 987
84Po [54Xe] 4f14 5d10 6s2 6p4 254 962](https://image.slidesharecdn.com/golonganoksigen-fix-111214090906-phpapp02/85/OXYGEN-3-320.jpg)
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OXYGEN
The document discusses various oxygen and sulfur compounds. It describes the characteristics of common oxygen groups like oxygen, ozone, hydrogen peroxide and their bonding structures. It also discusses the properties of sulfur and sulfur compounds such as hydrogen sulfide, sulfides, sulfur oxides, sulfuric acid, sulfur salts and sulfur halides. The document provides information on the tendencies and bonding preferences in these oxygen and sulfur compounds.
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OXYGEN
- 1. ulfa tessa selvi vici fala
- 2. Tendency Anomaly Sulfur Oxygen Oxygen groups Oxygen Covalent hydrogen Sulfide bond in oxygen compound Sulfide Tendency in the covalent Sulfur oxyde compound Sulfuric acid hydrogen peroxide Sulfur-oxide salt Sulfur halide
- 3. The Preference ofOxygen Groups Table 1. Data Of Some Oxygen Group Characteristic elements Electron Melting Boiling point configuration point (oC) (oC) 8O [2He] 2s2 2p4 -219 -183 16S [10Ne] 3s2 3p4 119 445 34Se [18Ar] 3d10 4s2 4p4 221 685 52Te [36Kr] 4d10 5s2 5p4 452 987 84Po [54Xe] 4f14 5d10 6s2 6p4 254 962
- 4. • Double bondstability and katenasi's character Double bond on oxygen much greater than its single bond, single bond O-O is very weak relevance with formation katenasi. In carbon groups (faction 14), katenasi’s ability is decrease with its increasing atomic number, but in groups 16, Sulfur can form the longest chain (S8). In fact, single bond O-O is weakest than single bond of oxygen atom with other atoms, O - X. Thus, oxygen atom prefers to form bonding with another atoms than with itself. • Its absents orbital d. Oxygen forms just one with fluorin's compound which is OF2, but sulfur can form some compound with fluorin include SF6. To reach until six its covalent bonds, sulfur atom have to involve orbital d. Thus, not be found flourin's oxygen compound that analog with SF6 because there is no orbital d in oxygen atom.
- 5. Dioxygen Trioxygen ( O2 ) ( O3 ) - Dark blue gas - colorless gases - Boiling point - 112 oC - Has boiling point – 183 oC - diamagnetic - its color is blue in the - Toxic gas liquid phase. - ozon produced by - paramagnetic SUTET, photocopy engine - reactive gas. and laser print. -The solubility is lower than - As oxidator that stronger carbondioxyde than O2.
- 6. The bonding inoxygen covalent compound oxygen Single Double Triple coordinate Bond Bond Bond bond angles between the two single covalent bonds maybe smaller Another way is oxygen atoms can than the regular tetrahedral form an equivalent three single angle (109o) it is influenced by covalent bond. a number of free electrons. Example of hydronium ion H3O+ example: Bond angle H-O-H are 104,5o
- 7. Tendency in oxygencompound Electropositive Electropositive Metal oxides with Nonmetal metal oxides metal oxides more than one oxides strong weak kind of oxide Have - Always bound characteristics Are oxides with low covalently ionic and basic. amphoteric. It oxidation levels - Nonmetals with low Examples : means can are alkaline. oxidation level are - BaO react with acid Oxides with high neutral - CuO (not and base. oxidation levels - Nonmetals with high soluble in water example : ZnO are acidic oxidation level are but soluble in acidic dilute acid)
- 8. Hydrogen Peroxide • Purehydrogen peroxide is almost colorless liquid. • Very viscous because of hydrogen bonding. • Corrosive. • Not stable. • Easily to disporpotionation according to reaction : 2 H2O2 (l) 2 H2O (l) + O2 (g) • Forming a dihedral with angle 111o and bond angle of H-O- O is 94,5o.
- 9. Sulfur • Forming anionic compound with the active metal. • Forming a covalent compound. • Single covalent bond length 104 pm. • Electronegativity 2,6 • Allotropes of Sulfur is S8 (cyclorooctasulfur), S6 (cyclorohexasulfur), and S12 (cyclododecasulfur).
- 10. S6 S12 is the most stable allotrope of sulfur that can be synthesized by mixing sodium thiosulfate solution Na2S2O3 with hydrochloric acid : 6Na2S2O3(aq) +12HCl(aq) → S6(s) + 6SO2(g) + 12NaCl(aq) + 6H2O(l)
- 11. Hydrogen Sulfide Characteristic : colorless gases its smell is bad like stinky egg toxic gas produced by anaerob bactery trough decomposition reaction. in laboratory gas H2S produced by reaction : FeS(s) + 2HCl(aq) FeCl2(aq) + H2S(g) can identified with Pb2S prodused brown black PbS
- 12. Sulfide • group 1,2, aluminium are dissolve in water. • S2-(aq) + H2O (l) HS- (aq) + OH – (aq) • Continued hydrolisis produce H2S gas that smells stinky : • HS - (aq) + H2O(l) H2S (s) + OH- (aq) • function of sulfide : in battery, cosmetics, etc.
- 13. Sulfur oxides Sulfur dioxide Sulfur trioxide Equilateral triangle stucture Nonlinier Stucture Easier dissolve in water Strong acidic and dissolve in water form sulfuric acid with reaction: SO3 (g) + H2O H2 SO4
- 14. Sulfuric Acid • Thickliquid like oil • Pure sulfuric acid has conductivity properties • Sulfuric acid can be react in 5 ways are: 1. As acid 2. Drying agent to water 3. Oxidation agent 4. Sulfonation agent 5. As base
- 15. 1. As acid Dilute sulfuric acid usually as acid 2. Drying agent to water Has ability to destroy water component from formula structure of a compound 3. Oxidation agent Hot concentrate sulfuric acid is good oxidation agent 4. Sulfonation agent Concentrate sulfuric acid has ability replaced 1 atom hydrogen in organic compound with sulfonic acid 5. As base Sulfuric acid can be base if added to stronger protone donor
- 16. Producing Sulfuric Acid •Producing methode according to contact process even lead chamber always using sulfur dioxide that can be prepared from sulfur melted combustion in dry air: • S (s) + O2 SO2(g) • Mixture sulfur dioxide with dry air flow into catalisator V2O5 at 400-500o C.
- 17. Sulfur-oxide Salt Sulfate isproduced with three step : Hydrogen 1. Between natrium sulfate is an Sulfite can be Thiosulfate hydroxyde with acidic, that can formed by dilute sulfuric acid can be formed be formed by flowing sulfur 2. Reaction between by boiling reaction dioxyde gas electropositive sulfur in between into natrium metal and dilute sulfate natrium hydroxyde sulforic acid aqueous 3. Reaction between hydroxyde with aqueous carbonate salt and sulfuric acid dilute sulfuric acid Peroksodisulfate ion has one dioxo bridge. Its acid is white solid, two important salt as oxidator agent are potassium and amonium peroksodisulfate, with peroksodisulfate ion is reductated become sulfate ion.
- 18. Sulfur Halide • Theimportant compound of sulfur-halogen are sulfur-fluorin, and sulfur-chlorine. • Sulfur-fluorin form SF6 (colorless gas, unsmell, not reactive, low toxic, stable) and SF4 (reactive gas, is decomposed by wet air become sulfur-dioxyde and hydrogen fluoride). • Sulfur-chlorin only form with low oxidation level. Sulfur melted that flowed with dichlorin gas producing disulfur dichloride, S2Cl2. disulfur dichoride much used in rubber vulcanization process.